274408
Cuprous ion is colourless while cupric ion is coloured because:
1 Both have half filled p-and d-orbitals.
2 Cuprous ion has incomplete d-orbitaland cupric ion has a complete d-orbital.
3 Both have unpaired electrons in the d-orbitals.
4 Cuprous ion has complete d-orbtal and cupric ion has an incomplete d-orbital.
Explanation:
(D) : $\mathrm{Cu}^{+}$ion has $\left(3 \mathrm{~d}^{10}\right)$ configuration while $\mathrm{Cu}^{2+}$ ion has $\left(3 \mathrm{~d}^{9}\right)$ configuration. In $\mathrm{Cu}^{+}$ion there is no $\mathrm{d}-\mathrm{d}$ transition while in $\mathrm{Cu}^{2+}, \mathrm{d}$-d transition is possible.
AIIMS-2012
COORDINATION COMPOUNDS
274410
The colour of copper sulphide is
1 Blue
2 Black
3 Red
4 Green
Explanation:
(A) : Crystal of copper sulphide is blue in colour because $\mathrm{Cu}^{2+}$ absorbs the wavelength of orange light and emits blue colour.
AIIMS-2010
COORDINATION COMPOUNDS
274413
The colour in the coordination compounds Can be readily explained in terms of
1 spectrochemical
2 chelate effect
3 crystal field theory
4 none of the above.
Explanation:
(C) : The Crystal Field Theory (CFT) is successful in explaining the formation structure colour and magnetic properties of coordination compounds to a large extent.
J and K CET-(2014)
COORDINATION COMPOUNDS
274418
Which of the following ions will exhibits colour in aqueous solutions?
1 $\mathrm{La}^{3+}(\mathrm{Z}=57)$
2 $\mathrm{Ti}^{3+}(\mathrm{Z}=22)$
3 $\mathrm{Lu}^{3+}(\mathrm{Z}=71)$
4 $\mathrm{Sc}^{3+}(\mathrm{Z}=21)$
Explanation:
(B) : $\mathrm{Ti}^{3+}(\mathrm{Z}=22) 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 4 \mathrm{~s}^{1} 3 \mathrm{~d}^{0}$ presence of an unpaired electron in the s-orbital of $\mathrm{Ti}^{3+}$ causes it to exhibit color in aqueous solution.
AIPMT -2010
COORDINATION COMPOUNDS
274425
Formation of coloured ions by transition metals signifies;
1 absorption of light from UV range
2 emission of light
3 presence of unpaired electrons in s and $\mathrm{p}$ orbitals
4 complimentary colours to the absorbed light
Explanation:
(D) : Transition metal ions have the property to absorb certain radiation from the visible region and exhibit the complementary colour.
274408
Cuprous ion is colourless while cupric ion is coloured because:
1 Both have half filled p-and d-orbitals.
2 Cuprous ion has incomplete d-orbitaland cupric ion has a complete d-orbital.
3 Both have unpaired electrons in the d-orbitals.
4 Cuprous ion has complete d-orbtal and cupric ion has an incomplete d-orbital.
Explanation:
(D) : $\mathrm{Cu}^{+}$ion has $\left(3 \mathrm{~d}^{10}\right)$ configuration while $\mathrm{Cu}^{2+}$ ion has $\left(3 \mathrm{~d}^{9}\right)$ configuration. In $\mathrm{Cu}^{+}$ion there is no $\mathrm{d}-\mathrm{d}$ transition while in $\mathrm{Cu}^{2+}, \mathrm{d}$-d transition is possible.
AIIMS-2012
COORDINATION COMPOUNDS
274410
The colour of copper sulphide is
1 Blue
2 Black
3 Red
4 Green
Explanation:
(A) : Crystal of copper sulphide is blue in colour because $\mathrm{Cu}^{2+}$ absorbs the wavelength of orange light and emits blue colour.
AIIMS-2010
COORDINATION COMPOUNDS
274413
The colour in the coordination compounds Can be readily explained in terms of
1 spectrochemical
2 chelate effect
3 crystal field theory
4 none of the above.
Explanation:
(C) : The Crystal Field Theory (CFT) is successful in explaining the formation structure colour and magnetic properties of coordination compounds to a large extent.
J and K CET-(2014)
COORDINATION COMPOUNDS
274418
Which of the following ions will exhibits colour in aqueous solutions?
1 $\mathrm{La}^{3+}(\mathrm{Z}=57)$
2 $\mathrm{Ti}^{3+}(\mathrm{Z}=22)$
3 $\mathrm{Lu}^{3+}(\mathrm{Z}=71)$
4 $\mathrm{Sc}^{3+}(\mathrm{Z}=21)$
Explanation:
(B) : $\mathrm{Ti}^{3+}(\mathrm{Z}=22) 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 4 \mathrm{~s}^{1} 3 \mathrm{~d}^{0}$ presence of an unpaired electron in the s-orbital of $\mathrm{Ti}^{3+}$ causes it to exhibit color in aqueous solution.
AIPMT -2010
COORDINATION COMPOUNDS
274425
Formation of coloured ions by transition metals signifies;
1 absorption of light from UV range
2 emission of light
3 presence of unpaired electrons in s and $\mathrm{p}$ orbitals
4 complimentary colours to the absorbed light
Explanation:
(D) : Transition metal ions have the property to absorb certain radiation from the visible region and exhibit the complementary colour.
274408
Cuprous ion is colourless while cupric ion is coloured because:
1 Both have half filled p-and d-orbitals.
2 Cuprous ion has incomplete d-orbitaland cupric ion has a complete d-orbital.
3 Both have unpaired electrons in the d-orbitals.
4 Cuprous ion has complete d-orbtal and cupric ion has an incomplete d-orbital.
Explanation:
(D) : $\mathrm{Cu}^{+}$ion has $\left(3 \mathrm{~d}^{10}\right)$ configuration while $\mathrm{Cu}^{2+}$ ion has $\left(3 \mathrm{~d}^{9}\right)$ configuration. In $\mathrm{Cu}^{+}$ion there is no $\mathrm{d}-\mathrm{d}$ transition while in $\mathrm{Cu}^{2+}, \mathrm{d}$-d transition is possible.
AIIMS-2012
COORDINATION COMPOUNDS
274410
The colour of copper sulphide is
1 Blue
2 Black
3 Red
4 Green
Explanation:
(A) : Crystal of copper sulphide is blue in colour because $\mathrm{Cu}^{2+}$ absorbs the wavelength of orange light and emits blue colour.
AIIMS-2010
COORDINATION COMPOUNDS
274413
The colour in the coordination compounds Can be readily explained in terms of
1 spectrochemical
2 chelate effect
3 crystal field theory
4 none of the above.
Explanation:
(C) : The Crystal Field Theory (CFT) is successful in explaining the formation structure colour and magnetic properties of coordination compounds to a large extent.
J and K CET-(2014)
COORDINATION COMPOUNDS
274418
Which of the following ions will exhibits colour in aqueous solutions?
1 $\mathrm{La}^{3+}(\mathrm{Z}=57)$
2 $\mathrm{Ti}^{3+}(\mathrm{Z}=22)$
3 $\mathrm{Lu}^{3+}(\mathrm{Z}=71)$
4 $\mathrm{Sc}^{3+}(\mathrm{Z}=21)$
Explanation:
(B) : $\mathrm{Ti}^{3+}(\mathrm{Z}=22) 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 4 \mathrm{~s}^{1} 3 \mathrm{~d}^{0}$ presence of an unpaired electron in the s-orbital of $\mathrm{Ti}^{3+}$ causes it to exhibit color in aqueous solution.
AIPMT -2010
COORDINATION COMPOUNDS
274425
Formation of coloured ions by transition metals signifies;
1 absorption of light from UV range
2 emission of light
3 presence of unpaired electrons in s and $\mathrm{p}$ orbitals
4 complimentary colours to the absorbed light
Explanation:
(D) : Transition metal ions have the property to absorb certain radiation from the visible region and exhibit the complementary colour.
274408
Cuprous ion is colourless while cupric ion is coloured because:
1 Both have half filled p-and d-orbitals.
2 Cuprous ion has incomplete d-orbitaland cupric ion has a complete d-orbital.
3 Both have unpaired electrons in the d-orbitals.
4 Cuprous ion has complete d-orbtal and cupric ion has an incomplete d-orbital.
Explanation:
(D) : $\mathrm{Cu}^{+}$ion has $\left(3 \mathrm{~d}^{10}\right)$ configuration while $\mathrm{Cu}^{2+}$ ion has $\left(3 \mathrm{~d}^{9}\right)$ configuration. In $\mathrm{Cu}^{+}$ion there is no $\mathrm{d}-\mathrm{d}$ transition while in $\mathrm{Cu}^{2+}, \mathrm{d}$-d transition is possible.
AIIMS-2012
COORDINATION COMPOUNDS
274410
The colour of copper sulphide is
1 Blue
2 Black
3 Red
4 Green
Explanation:
(A) : Crystal of copper sulphide is blue in colour because $\mathrm{Cu}^{2+}$ absorbs the wavelength of orange light and emits blue colour.
AIIMS-2010
COORDINATION COMPOUNDS
274413
The colour in the coordination compounds Can be readily explained in terms of
1 spectrochemical
2 chelate effect
3 crystal field theory
4 none of the above.
Explanation:
(C) : The Crystal Field Theory (CFT) is successful in explaining the formation structure colour and magnetic properties of coordination compounds to a large extent.
J and K CET-(2014)
COORDINATION COMPOUNDS
274418
Which of the following ions will exhibits colour in aqueous solutions?
1 $\mathrm{La}^{3+}(\mathrm{Z}=57)$
2 $\mathrm{Ti}^{3+}(\mathrm{Z}=22)$
3 $\mathrm{Lu}^{3+}(\mathrm{Z}=71)$
4 $\mathrm{Sc}^{3+}(\mathrm{Z}=21)$
Explanation:
(B) : $\mathrm{Ti}^{3+}(\mathrm{Z}=22) 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 4 \mathrm{~s}^{1} 3 \mathrm{~d}^{0}$ presence of an unpaired electron in the s-orbital of $\mathrm{Ti}^{3+}$ causes it to exhibit color in aqueous solution.
AIPMT -2010
COORDINATION COMPOUNDS
274425
Formation of coloured ions by transition metals signifies;
1 absorption of light from UV range
2 emission of light
3 presence of unpaired electrons in s and $\mathrm{p}$ orbitals
4 complimentary colours to the absorbed light
Explanation:
(D) : Transition metal ions have the property to absorb certain radiation from the visible region and exhibit the complementary colour.
274408
Cuprous ion is colourless while cupric ion is coloured because:
1 Both have half filled p-and d-orbitals.
2 Cuprous ion has incomplete d-orbitaland cupric ion has a complete d-orbital.
3 Both have unpaired electrons in the d-orbitals.
4 Cuprous ion has complete d-orbtal and cupric ion has an incomplete d-orbital.
Explanation:
(D) : $\mathrm{Cu}^{+}$ion has $\left(3 \mathrm{~d}^{10}\right)$ configuration while $\mathrm{Cu}^{2+}$ ion has $\left(3 \mathrm{~d}^{9}\right)$ configuration. In $\mathrm{Cu}^{+}$ion there is no $\mathrm{d}-\mathrm{d}$ transition while in $\mathrm{Cu}^{2+}, \mathrm{d}$-d transition is possible.
AIIMS-2012
COORDINATION COMPOUNDS
274410
The colour of copper sulphide is
1 Blue
2 Black
3 Red
4 Green
Explanation:
(A) : Crystal of copper sulphide is blue in colour because $\mathrm{Cu}^{2+}$ absorbs the wavelength of orange light and emits blue colour.
AIIMS-2010
COORDINATION COMPOUNDS
274413
The colour in the coordination compounds Can be readily explained in terms of
1 spectrochemical
2 chelate effect
3 crystal field theory
4 none of the above.
Explanation:
(C) : The Crystal Field Theory (CFT) is successful in explaining the formation structure colour and magnetic properties of coordination compounds to a large extent.
J and K CET-(2014)
COORDINATION COMPOUNDS
274418
Which of the following ions will exhibits colour in aqueous solutions?
1 $\mathrm{La}^{3+}(\mathrm{Z}=57)$
2 $\mathrm{Ti}^{3+}(\mathrm{Z}=22)$
3 $\mathrm{Lu}^{3+}(\mathrm{Z}=71)$
4 $\mathrm{Sc}^{3+}(\mathrm{Z}=21)$
Explanation:
(B) : $\mathrm{Ti}^{3+}(\mathrm{Z}=22) 1 \mathrm{~s}^{2} 2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2} 3 \mathrm{p}^{6} 4 \mathrm{~s}^{1} 3 \mathrm{~d}^{0}$ presence of an unpaired electron in the s-orbital of $\mathrm{Ti}^{3+}$ causes it to exhibit color in aqueous solution.
AIPMT -2010
COORDINATION COMPOUNDS
274425
Formation of coloured ions by transition metals signifies;
1 absorption of light from UV range
2 emission of light
3 presence of unpaired electrons in s and $\mathrm{p}$ orbitals
4 complimentary colours to the absorbed light
Explanation:
(D) : Transition metal ions have the property to absorb certain radiation from the visible region and exhibit the complementary colour.
